Some Basic Concepts of Chemistry - Result Question 46
####46. $10 g$ of hydrogen and $64 g$ of oxygen were filled in a steel vessel and exploded. Amount of water produced in this reaction will be:
(a) $3 mol$
(b) $4 mol$
(c) $1 mol$
(d) $2 mol$
[2009]
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Solution:
- (b)
$ \underset{\substack{10 mol)}}{H_2}+\underset{(2 mol)}{\frac{1}{2} O_2} \longrightarrow \underset{g}{H_2 O} $
In this reaction oxygen is the limiting agent.
Hence, amount of $H_2 O$ produced depends on the amount of $O_2$ taken.
$\because 0.5$ mole of $O_2$ gives $H_2 O=1 mol$
$\therefore 2$ mole of $O_2$ gives $H_2 O=4 mol$
When there is not enough of one reactant in a chemical reaction, the reaction stops. To find the amount of product produced, we must determine reactant that will limit the chemical reaction (the limiting reagent) we can find the limiting reagent by calculating the amount of product that can be formed by each reactant, the one that produces less product is the limiting reagent.
